How metals and non-metals transfer electrons to form ions, working out the charges from the periodic table, dot and cross diagrams, and why giant ionic lattices behave as they do.
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1.Name the three types of strong chemical bond.
Ionic, covalent and metallic.
2.Between which types of element does ionic bonding occur?
Between a metal and a non-metal.
3.What happens to electrons during ionic bonding?
They are transferred from the metal atom to the non-metal atom.
4.Why does a metal atom form a positive ion?
It loses electrons from its outer shell, so it then has more protons than electrons.
5.Why does a non-metal atom form a negative ion?
It gains electrons into its outer shell, so it then has more electrons than protons.
6.Why do atoms form ions at all?
To achieve a full outer shell, giving them the stable electronic structure of a noble gas.
7.What charge do Group 1 ions have?
1+, because they lose their single outer electron.
8.What charge do Group 2 ions have?
2+, because they lose two outer electrons.
9.What charge do Group 6 ions have?
2-, because they gain two electrons.
10.What charge do Group 7 ions have?
1-, because they gain one electron.
11.Define an ionic bond.
The strong electrostatic force of attraction between oppositely charged ions, acting in all directions.
12.Sodium has the structure 2,8,1. What ion does it form?
Na+, with the structure 2,8.
13.Oxygen has the structure 2,6. What ion does it form?
O2-, with the structure 2,8.
14.Does the number of protons change when an ion forms?
No. Only electrons are lost or gained, so the element stays the same.
15.What does a dot and cross diagram show?
The outer electrons of each atom, using dots for one atom and crosses for the other, so you can see where each electron came from.
16.Give a limitation of dot and cross diagrams.
They do not show the relative sizes of the ions, or how the ions are arranged in space.
17.What structure do ionic compounds have?
A giant ionic lattice: a regular repeating arrangement of oppositely charged ions.
18.Why do ionic compounds have high melting and boiling points?
There are many strong electrostatic forces of attraction acting in all directions between the oppositely charged ions, and a lot of energy is needed to overcome them.
19.Do ionic compounds conduct electricity when solid?
No. The ions are held in fixed positions in the lattice, so no charged particles are free to move.
20.When do ionic compounds conduct electricity?
When molten or dissolved in water, because the ions are then free to move and carry the charge.
21.Why is magnesium oxide higher melting than sodium chloride?
Its ions carry greater charges, 2+ and 2-, so the electrostatic attraction between them is stronger.
22.What is the formula of magnesium chloride, and why?
MgCl2. Magnesium forms a 2+ ion and chlorine forms a 1- ion, so two chloride ions are needed to balance the charge.
23.What is the formula of calcium oxide?
CaO. Calcium forms 2+ and oxygen forms 2-, so they balance one to one.
24.What does the formula of an ionic compound represent?
The simplest whole number ratio of the ions present, not the actual number in the lattice.
25.Give an advantage of a ball and stick model.
It shows how the ions are arranged in three dimensions and the shape of the lattice.
26.Give a limitation of a ball and stick model.
It suggests there are gaps between the ions and shows them far too small relative to the spacing, when in reality they are packed closely together.
27.What is an electrostatic force of attraction?
The force of attraction between particles carrying opposite charges.
28.Why are ionic compounds usually solid at room temperature?
The forces holding the lattice together are very strong, so a great deal of energy is needed before the particles can move freely.
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